Is the oxidation of a mineral that contains iron is an example of a mechanical or chemical

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Answer 1

The oxidation of a mineral containing iron is an example of a chemical process rather than a mechanical one.

Oxidation refers to a chemical reaction where a substance reacts with oxygen. In the case of iron, when it is exposed to oxygen in the presence of moisture or water, it undergoes a chemical reaction known as rusting or oxidation. This reaction forms iron oxide, commonly known as rust.

Mechanical processes, on the other hand, involve physical actions or movements rather than chemical reactions. Examples of mechanical processes include grinding, crushing, or breaking apart a mineral into smaller pieces, but these processes do not involve the chemical transformation of the mineral's composition.

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Related Questions

High-energy molecules contain one or more high-energy bonds, when hydrolyzed, is accompanied by a ______________ in free energy.

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High-energy molecules contain one or more high-energy bonds, which store energy that can be released through hydrolysis. Hydrolysis is a chemical reaction that involves the breaking of a molecule with the addition of water. When high-energy bonds are hydrolyzed, the reaction is accompanied by a decrease in free energy.

During hydrolysis, the high-energy bond in the molecule is broken, releasing energy. This energy is used to form new bonds with the water molecules, resulting in the formation of new compounds. The breaking of the high-energy bond and the formation of new bonds with water molecules require energy, which leads to a decrease in free energy.

To illustrate this concept, let's consider the hydrolysis of ATP (adenosine triphosphate), which is a high-energy molecule commonly used as a source of energy in cells. When ATP is hydrolyzed, one of its phosphate groups is cleaved off, forming ADP and inorganic phosphate (Pi). This hydrolysis reaction releases energy that can be used by cells to perform various cellular processes.

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a large volume of 0.1590 m h2so3(aq) is treated with enough naoh(s) to adjust the ph of the solution to 5.63 . assuming that the addition of naoh(s) does not significantly affect the volume of the solution, calculate the final molar concentrations of h2so3(aq) , hso−3(aq) , and so2−3(aq) in solution given that the Ka1 and Ka2 values are 1.50×10−2 and 1.20×10−7 , respectively.

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To calculate the final molar concentrations of H2SO3(aq), HSO−3(aq), and SO2−3(aq) in solution, we need to consider the dissociation of H2SO3. H2SO3(aq) can dissociate into HSO−3(aq) and H+(aq), and further into SO2−3(aq) and H+(aq).

Given that the Ka1 and Ka2 values are 1.50×10−2 and 1.20×10−7, respectively. Calculate the initial concentration of H2SO3(aq) using its volume and molarity. Use the Ka1 value to calculate the concentration of HSO−3(aq) and H+(aq) at equilibrium.

Subtract the concentration of H+(aq) from the initial concentration of H2SO3(aq) to find the final concentration of H2SO3(aq). Calculate the final concentration of HSO−3(aq) and SO2−3(aq) by subtracting the concentration of H+(aq) from their respective equilibrium concentrations.

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30 ml of 0. 00138 m cl- solution is titrated with 0. 00057 m ag+. calculate the pag half-way to the equivalence point when the added titrant volume is 30ml. (hint!: use the ksp value for agcl)

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The pAg halfway to the equivalence point when the added titrant volume is 30 ml is 7.45.

The pAg halfway to the equivalence point can be calculated using the concept of stoichiometry and the equilibrium constant expression for the formation of silver chloride (AgCl).

First, we need to determine the number of moles of Cl- present in the initial solution. The initial concentration of Cl- is 0.00138 M, and the volume of the solution is 30 ml. Therefore, the moles of Cl- can be calculated as follows:

Moles of Cl- = Concentration of Cl- × Volume of Solution

= 0.00138 M × 0.030 L

= 0.0000414 moles

Since the stoichiometry between Ag+ and Cl- is 1:1, the moles of Ag+ required to react with the moles of Cl- can be assumed to be the same.

Next, we calculate the concentration of Ag+ required to react with the moles of Cl-. The moles of Ag+ can be determined as follows:

Moles of Ag+ = Concentration of Ag+ × Volume of Titrant Added

= 0.00057 M × 0.030 L

= 0.0000171 moles

At the halfway point, the moles of Ag+ reacted with the moles of Cl- are equal. Therefore, the moles of Ag+ remaining in solution are:

Moles of Ag+ remaining = Moles of Ag+ initial - Moles of Ag+ reacted

= 0.0000171 moles - 0.0000414 moles

= -0.0000243 moles

Since the moles of Ag+ cannot be negative, we assume that all the Cl- ions have reacted, and the excess Ag+ ions have formed a precipitate of AgCl.

Using the equilibrium constant expression for AgCl, Ksp = [Ag+][Cl-], we can calculate the concentration of Ag+ at the halfway point.

Ksp = [Ag+][Cl-]

[Ag+] = Ksp / [Cl-]

= (1.77 × 10^-10) / (0.00138 M)

≈ 1.285 × 10^-7 M

Finally, we can calculate the pAg halfway to the equivalence point using the formula:

pAg = -log10([Ag+])

= -log10(1.285 × 10^-7)

≈ 7.45

Step 3: At the halfway point, all the Cl- ions have reacted with Ag+ ions to form AgCl. The remaining Ag+ ions in solution will be in equilibrium with the AgCl precipitate. The concentration of Ag+ at this point can be calculated using the equilibrium constant expression for AgCl.

The pAg halfway to the equivalence point is 7.45. This means that the concentration of Ag+ ions in the solution is approximately 1.285 × 10^-7 M. At this concentration, the solution is close to the solubility product constant (Ksp) for AgCl, which is 1.77 × 10^-10.

The pAg value represents the negative logarithm of the Ag+ concentration in the solution. By calculating the concentration of Ag+ at the halfway point, we can determine the pAg value.

The result indicates that halfway to the equivalence point, the concentration of Ag+ ions in the solution is relatively high, indicating that a significant portion of the AgCl precipitate has formed. This corresponds to the formation of a visible white precip

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at constant temperature, a 144.0 ml sample of gas in a piston chamber has a pressure of 2.25 atm. calculate the pressure of the gas if this piston is pushed down hard so that the gas now has a volume of 36.0 ml.

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The pressure of the gas would be 9.0 atm if the piston is pushed down hard to a volume of 36.0 ml.

To solve this problem, we can use Boyle's Law, which states that the pressure of a gas is inversely proportional to its volume at constant temperature.

First, we need to set up the equation: P1V1 = P2V2, where P1 and V1 are the initial pressure and volume, and P2 and V2 are the final pressure and volume.

Given that the initial volume (V1) is 144.0 ml and the initial pressure (P1) is 2.25 atm, and the final volume (V2) is 36.0 ml, we can plug in the values into the equation:

2.25 atm * 144.0 ml = P2 * 36.0 ml

Next, we can solve for P2 by dividing both sides of the equation by 36.0 ml:

2.25 atm * 144.0 ml / 36.0 ml = P2

P2 = 9.0 atm

Therefore, the pressure of the gas would be 9.0 atm if the piston is pushed down hard to a volume of 36.0 ml.

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the atomic weight of hydrogen is 1.008 amu. what is the percent composition of hydrogen by isotope, assuming that hydrogen’s only isotopes are 1h and 2d?

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The percent composition of hydrogen by isotope can be calculated based on the relative abundance of each isotope and their respective atomic masses. In this case, hydrogen has two isotopes: 1H and 2D Percent composition = (0.0002 * 2.014 amu) / [(0.9998 * 1.008 amu) + (0.0002 * 2.014 amu)]

To find the percent composition, we need to consider the relative abundance of each isotope. 1H is the most common isotope of hydrogen, with an abundance of approximately 99.98%. Its atomic mass is 1.002D, also known as deuterium, is the less common isotope, with an abundance of approximately 0.02%. Its atomic mass is 2.014 amu.To calculate the percent composition of each isotope, we can use the following formula:Percent composition = (Abundance * Atomic mass) / Average atomic massLet's calculate the percent composition for each isotope:

1HPercent composition = (0.9998 * 1.008 amu) / Average atomic mas2Percent composition = (0.0002 * 2.014 amu) / Average atomic massTo find the average atomic mass, we can use the weighted average formula:Average atomic mass = (Abundance of 1H * Atomic mass of 1H) + (Abundance of 2D * Atomic mass of 2D)Substituting the values, we get:

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A graduated cylinder contains 26 cm3 of water. an object with a mass of 21 grams and a volume of 15 cm3 is lowered into the water. what will the new water level be

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When the object with a volume of 15 cm3 is lowered into the water in the graduated cylinder, the new water level will be 11 cm3.

The new water level in the graduated cylinder can be determined by considering the principle of displacement. When the object is lowered into the water, it will displace an amount of water equal to its own volume.

Given that the object has a volume of 15 cm3, it will displace 15 cm3 of water. Since the initial volume of water in the graduated cylinder is 26 cm3, the new water level can be calculated by subtracting the volume of water displaced by the object from the initial volume of water.

Therefore, the new water level in the graduated cylinder will be 26 cm3 - 15 cm3 = 11 cm3.

To summarize, when the object with a volume of 15 cm3 is lowered into the water in the graduated cylinder, the new water level will be 11 cm3.

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a homogeneous solution contains copper(ii) ions (cu2 ), silver ions (ag ) and potassium ions (k ). you have sodium bromide (nabr) and sodium sulfide (na2s) available to use. what should you add and in what order to separate the three metal ions? ksp (sulfides) ksp (bromides) cus 6.0×10–37 cubr2 soluble ag2s 6.0×10–51 agbr 7.7×10–13 k2s soluble kbr soluble

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To separate Cu2+, Ag+, and K+ from the homogeneous solution, add sodium sulfide (Na2S) first to precipitate CuS. Then add sodium bromide (NaBr) to precipitate AgBr. Finally, the remaining solution contains only K+.

To separate the copper (II), silver, and potassium ions from the homogeneous solution, you can employ the following procedure.

Firstly, add sodium sulfide (Na2S) to the solution, resulting in the formation of insoluble copper sulfide (CuS) precipitate due to its low solubility (Ksp = 6.0×10–37). By filtering the solution, the insoluble CuS precipitate can be separated.

Next, introduce sodium bromide (NaBr) to the filtrate, causing the formation of insoluble silver bromide (AgBr) precipitate due to its low solubility (Ksp = 7.7×10–13). By filtering the solution once again, the insoluble AgBr precipitate can be isolated.

Finally, the remaining solution will only contain potassium ions (K+), which do not require further separation steps as potassium salts are highly soluble in water. By following this procedure, effective separation of the copper (II), silver, and potassium ions can be achieved.

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You prepare a stock solution that has a concentration of 2. 5 m. An aliquot with a volume of 10. 0 ml is removed from the solution. What is the concentration of the aliquot?.

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The concentration of the aliquot is 2.5 M.

The concentration of a solution is defined as the amount of solute present per unit volume of the solution.

In this case, the stock solution has a concentration of 2.5 M (moles per liter).

An aliquot is a small portion or sample taken from a larger solution. In this scenario, an aliquot with a volume of 10.0 ml is removed from the stock solution.

Since the concentration of the stock solution is given in terms of moles per liter (M), the concentration of the aliquot will be the same as the concentration of the stock solution.

The concentration does not change when a specific volume is removed from the solution.

Therefore, the concentration of the aliquot is 2.5 M. It is important to note that the concentration remains the same regardless of the volume of the aliquot, as long as the proportion of solute to solvent remains constant.

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